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A container holds 192 g of oxygen gas at a pressure of 8.00 atm.
How much heat Q is required to increase the temperature by
145 °C at constant volume?

Sagot :

Lanuel

The quantity of heat (Q) that is required to increase the temperature at constant volume is 18,082.95 Joules.

Given the following data:

  • Mass of oxygen gas = 192 g
  • Pressure = 8.00 atm
  • Temperature = 145°C

Scientific data:

  • Ideal gas constant, R = 8.314 J/molK
  • Molar mass of oxygen gas = 32 g/mol.

To determine the quantity of heat (Q) that is required to increase the temperature at constant volume:

First of all, we would find the number of moles of oxygen gas.

[tex]Number\;of\;moles = \frac{mass}{molar\;mass}\\\\Number\;of\;moles = \frac{192}{32}[/tex]

Number of moles = 6 moles.

At constant volume, the heat capacity for a diatomic gas is given by:

[tex]C_v = \frac{5}{2} R\\\\C_v =\frac{5}{2} \times 8.314[/tex]

Heat capacity = 20.785 J/molK.

At constant volume, the quantity of heat (Q) is given by this formula:

[tex]Q = nC_v \Delta T\\\\Q=6 \times 20.785 \times 145[/tex]

Quantity of heat (Q) = 18,082.95 Joules

Note: [tex]\Delta T[/tex] = 145°C = 145 K (since the difference is the same).

Read more on heat capacity here: https://brainly.com/question/11150071

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